Question 15.1: Account for the acidic properties of nitrous acid (HNO2) usi......
Account for the acidic properties of nitrous acid (HNO_{2}) using the Arrhenius theory and the Brønsted–Lowry theory, and identify the conjugate base of HNO_{2}.
STRATEGY
To account for the acidity of a substance, consider how it can produce H^{+} ions in water (Arrhenius theory) and how it can act as a proton donor (Brønsted–Lowry theory).
Step-by-Step
HNO_{2} is an Arrhenius acid because it dissociates in water to produce H^{+} ions:
HNO_{2}(aq)\xrightleftharpoons{}H^{+}(aq)+NO_{2} ^{-}(aq)Nitrous acid is a Brønsted–Lowry acid because it acts as a proton donor when it dissociates, transferring a proton to water to give the hydronium ion, H_{3}O^{+}:
The conjugate base of HNO_{2} is NO_{2} ^{-}, the species that remains after HNO_{2} has lost a proton.
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